In the combustion of carbon, how many grams of oxygen (O_2) are required to produce 37.15 g of carbon dioxide (CO_2)?C + O_2 → CO_2

• A. 16.00 g
• B. 44.00 g
• C. 27.09 g
• D. 32.00 g

Answer: (C)

Verified step by step guidance

1. Write the balanced chemical equation for the combustion of carbon: \(\mathrm{C} + \mathrm{O}_2 \rightarrow \mathrm{CO}_2\).
2. Calculate the number of moles of \(\mathrm{CO}_2\) produced using its molar mass: \(\text{moles of } \mathrm{CO}_2 = \frac{37.15\ \mathrm{g}}{44.00\ \mathrm{g/mol}}\).
3. Use the mole ratio from the balanced equation to find the moles of \(\mathrm{O}_2\) required. According to the equation, 1 mole of \(\mathrm{CO}_2\) is produced from 1 mole of \(\mathrm{O}_2\), so moles of \(\mathrm{O}_2 = \) moles of \(\mathrm{CO}_2\).
4. Calculate the mass of \(\mathrm{O}_2\) needed by multiplying the moles of \(\mathrm{O}_2\) by its molar mass: \(\text{mass of } \mathrm{O}_2 = \text{moles of } \mathrm{O}_2 \times 32.00\ \mathrm{g/mol}\).
5. The result from the previous step gives the grams of oxygen required to produce 37.15 g of carbon dioxide.